UNIT 1 Classification of Matter/ The Underlying Structure of Matter
NB Prescribed Outcomes
Students will be expected to:
define and classify matter according to its composition (pure substances or mixtures).
define and distinguish between, chemical and physical properties.
define and classify matter as elements and compounds, and as heterogeneous mixtures and solutions.
use the periodic law as illustrated by the periodic table to identify and distinguish metals and non-metals, periods and groups, representative and transition elements, and
describe the factors which contribute to the unique position of hydrogen on the periodic table.
identify the elements that are most prevalent in living systems.
research ingredients and additives in consumer products. (213-7)
identify consumer products and investigate the claims made by companies about the products. (212-5)
use standard atomic notation to represent atoms, define isotope and use isotopic notation.
predict ionic charges from position on the Periodic Table.
define atomic mass, explain the relative nature of atomic mass.
provide definitions and examples of atoms, ions, and molecules, including subatomic particles, atomic mass, atomic number, mass number, valence electrons, isotopes.
identify the inadequacies in the Rutherford and Bohr models.
identify the new proposal in the Bohr model of the atom.
describe the energies and positions of electrons according to the quantum mechanical model
describe how the shapes of orbitals differ as it relates to different sublevels.
write electron configuration diagrams using Hund‟ rule, Pauli exclusion principle and Aufbau principle (diagonal rule).
UNIT 4 Solutions and Water Properties
Ch 11.3/15.1/15.2/Ch7/16.1/16.2 Students will be expected to: - identify and describe the properties of ionic, molecular, metallic and covalent network substances. (321-7) -classify ionic, molecular, metallic and covalent network substances according to their properties. (321-9) -describe how the different types of bonds account for the properties of ionic, molecular, metallic and covalent network substances. (321-8) -illustrate and explain the formation of ionic, covalent, and metallic bonds (321-4b) -define valence electrons, electronegativity, ionic, metallic bond, nonpolar covalent and polar covalent bond. -identify lone pairs, bonding electrons, deduce bonding -capacity, sketch Lewis Dot structures and structural diagrams. -identify limitations of categorizing bond types based on differences in electronegativity between the elements and compounds (214-2) -investigate covalent network solids with reference to the allotropes of carbon (diamond, graphite, fullerenes, Bucky ball, nanotubes). -use library and electronic research tools to collect bonding information. (213-6) -select and integrate information from various print and electronic sources. (213-7) -compile and organize solution data, using appropriate formats and data treatments to facilitate interpretation of solubility. (213-5) -explain solubility, using the concept of equilibrium. (323-4) -identify different types of solutions (acids, bases, neutral, ionic and molecular) and their properties (conductivity, pH, solubility). -identify dissociation and ionization equations. -use the solubility generalizations to predict the formation of precipitates. (323-8) -conduct a precipitate lab and include recording, observing and collecting data, writing ionic and net ionic equations, and analyzing results.
-determine the molar solubility of a pure substance in water. (322-6)
calculate the concentration in mol/L or molarity, M, of solutions based on mass and/or moles of the solute (or solute ions) and volume of the solution.
- calculate concentration as %weight/volume (%w/v), % volume and parts per million (ppm). - practice preparation of a standard from a solid, and performing a dilution to produce a standard solution.
- know that [ ] always implies concentration in mol/L. - perform experiments involving the creation of stock solutions and relevant calculations. - perform experiments involving dilutions and relevant dilution calculations.
-identify and describe science-and technology-based careers related to solutions and equilibrium. (117-7) Chemistry 111 -differentiate between molarity and molality.
-demonstrate an understanding of colligative properties.
-explain the variations in the solubility of various pure substances, given the same solvent. (323-7) – explain the factors that affect dissolving and the rate of dissolving (temperature, pressure etc.). – explain how ionic and molecular compounds form solutions by relating the dissolution to intermolecular forces and forces of attraction. – describe the solubility of ionic and molecular compounds in polar and nonpolar solvents. – develop an understanding that solutions are mixtures formed by the physical mixing at the particle level and do not involve a chemical change.
NB Prescribed Outcomes
Students will be expected to:
define and classify matter according to its composition (pure substances or mixtures).
define and distinguish between, chemical and physical properties.
define and classify matter as elements and compounds, and as heterogeneous mixtures and solutions.
use the periodic law as illustrated by the periodic table to identify and distinguish metals and non-metals, periods and groups, representative and transition elements, and
describe the factors which contribute to the unique position of hydrogen on the periodic table.
identify the elements that are most prevalent in living systems.
research ingredients and additives in consumer products. (213-7)
identify consumer products and investigate the claims made by companies about the products. (212-5)
use standard atomic notation to represent atoms, define isotope and use isotopic notation.
predict ionic charges from position on the Periodic Table.
define atomic mass, explain the relative nature of atomic mass.
provide definitions and examples of atoms, ions, and molecules, including subatomic particles, atomic mass, atomic number, mass number, valence electrons, isotopes.
identify the inadequacies in the Rutherford and Bohr models.
identify the new proposal in the Bohr model of the atom.
describe the energies and positions of electrons according to the quantum mechanical model
describe how the shapes of orbitals differ as it relates to different sublevels.
write electron configuration diagrams using Hund‟ rule, Pauli exclusion principle and Aufbau principle (diagonal rule).
UNIT 4 Solutions and Water Properties
Ch 11.3/15.1/15.2/Ch7/16.1/16.2
Students will be expected to:
- identify and describe the properties of ionic, molecular, metallic and covalent network substances. (321-7)
-classify ionic, molecular, metallic and covalent network substances according to their properties.
(321-9)
-describe how the different types of bonds account for the properties of ionic, molecular, metallic and covalent network substances. (321-8)
-illustrate and explain the formation of ionic, covalent, and metallic bonds (321-4b)
-define valence electrons, electronegativity, ionic, metallic bond, nonpolar covalent and polar covalent bond.
-identify lone pairs, bonding electrons, deduce bonding -capacity, sketch Lewis Dot structures and structural diagrams.
-identify limitations of categorizing bond types based on differences in electronegativity between the elements and compounds (214-2)
-investigate covalent network solids with reference to the allotropes of carbon (diamond, graphite, fullerenes, Bucky ball, nanotubes).
-use library and electronic research tools to collect bonding information. (213-6)
-select and integrate information from various print and electronic sources. (213-7)
-compile and organize solution data, using appropriate formats and data treatments to facilitate interpretation of solubility. (213-5)
-explain solubility, using the concept of equilibrium. (323-4)
-identify different types of solutions (acids, bases, neutral, ionic and molecular) and their properties (conductivity, pH, solubility).
-identify dissociation and ionization equations.
-use the solubility generalizations to predict the formation of precipitates. (323-8)
-conduct a precipitate lab and include recording, observing and collecting data, writing ionic and net ionic equations, and analyzing results.
-determine the molar solubility of a pure substance in water. (322-6)
calculate the concentration in mol/L or molarity, M, of solutions based on mass and/or moles of the solute (or solute ions) and volume of the solution.
- calculate concentration as %weight/volume (%w/v), % volume and parts per million (ppm).
- practice preparation of a standard from a solid, and performing a dilution to produce a standard solution.
- know that [ ] always implies concentration in mol/L.
- perform experiments involving the creation of stock solutions and relevant calculations.
- perform experiments involving dilutions and relevant dilution calculations.
-identify and describe science-and technology-based careers related to solutions and equilibrium. (117-7)
Chemistry 111
-differentiate between molarity and molality.
-demonstrate an understanding of colligative properties.
-explain the variations in the solubility of various pure substances, given the same solvent. (323-7)
– explain the factors that affect dissolving and the rate of dissolving (temperature, pressure etc.).
– explain how ionic and molecular compounds form solutions by relating the dissolution to intermolecular forces and forces of attraction.
– describe the solubility of ionic and molecular compounds in polar and nonpolar solvents.
– develop an understanding that solutions are mixtures formed by the physical mixing at the particle level and do not involve a chemical change.
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